The correct order of increasing bond angles in the following triatomic species is

According to VSEPR theory, The order of repulsion of electrons is lp-lp repulsion gt lp-bp repulsion gt bp-bp repulsion Higher the number of lone pair of electrons (greater is repulsion ) lower is the bond angle and vice-versa. In $N{O}_2^{-}$ one lone pair of electron is present while in $N{O}_2^{+}$ no lone pair of electron is present. Hence the correct order of bond angles is $N{O}_2^{-}<N{O}_2<N{O}_2^{+}$